Calculate the entropy of HBr at 298 K and 1.00 bar, given that the bond length is 1.41 Å and the masses of ¹H and 79Br are 1.008 amu and 78.92 amu, respectively. The vibrational wavenumber is 2649 cm-¹. ep 1 of 7 Provide the equation needed to calculate the translational contribution to the total entropy. (Use the following as necessary: h, kg, m to represent the mass, P, T, and T.) Strans = R In (21mkT) h³ P (2mmkgT) kgT P ep 2 of 7 Substitute numerical values into the equation from Step 1 to obtain a numerical calculation for the translational entropy contribution. XJ-K-1.mol-1 Strans=146.211 Submit

Calculate the entropy of HBr at 298 K and 1.00 bar, given that the bond length is 1.41 Å and the masses of ¹H and 79Br are 1.008 amu and 78.92 amu, respectively. The vibrational wavenumber is 2649 cm-¹. ep 1 of 7 Provide the equation needed to calculate the translational contribution to the total entropy. (Use the following as necessary: h, kg, m to represent the mass, P, T, and T.) Strans = R In (21mkT) h³ P (2mmkgT) kgT P ep 2 of 7 Substitute numerical values into the equation from Step 1 to obtain a numerical calculation for the translational entropy contribution. XJ-K-1.mol-1 Strans=146.211 Submit

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Derivation Calculate the entropy of HBr at 298 K and 1.00 bar, given that the bond length is 1.41 Å and the masses of ¹H and 79Br are 1.008 amu and 78.92 amu, respectively. The vibrational wavenumber is 2649 cm-¹. Step 1 of 7 Provide the equation needed to calculate the translational contribution to the total entropy. (Use the following as necessary: h, kB, m to represent the mass, P, T, and T.) (²³1) (2πmkT) h³ Strans = R In kµT (²/2) e P (2πmkBT) ³ kBT h³ P Step 2 of 7 Substitute numerical values into the equation from Step 1 to obtain a numerical calculation for the translational entropy contribution. Strans = 163.61 163.484901080763 J.K-1.mol-1 Step 3 of 7 Provide the equation needed to calculate the rotational contribution to the total entropy. (Use the following as necessary: h, I, kB, 7, σ, and T.) Srot = R In 8n²lkpT oh² + R 87² IkBT oh² Step 4 of 7 Substitute numerical values into the equation from Step 3 to obtain a numerical calculation for the rotational entropy…
At 298K, the enthalpy of denaturation (unfolding) of hen egg whites lysozyme is +112.6 kJ/mol and the change in the constant pressure molar heat capacity resulting from the denaturation fo hte protein is +12.1 kJ/molK. Calculate the entropy of denaturation of hen eggs white lysoenyme at 360K (the melting or folding temperature of the enzyme) in units of kJ/molK
A2 Calculate the change in molar entropy of trichloromethane when heated from 0.00C to 270C. The constant pressure molar heat capacity fits the expression 91.47 + 7.5 × 10-2(T/K) between 240 K and 330 K.
Determine the standard molar entropy of N2 (ν˜ = 2359 cm−1 , B = 2.00 cm−1 and electronic ground state has degeneracy 1 under standard thermodynamic conditions. You can assume ideal gas behaviour. 1. Calculate the standard internal molar energy U 2. Calculate the standard molar entropy S (standard thermodynamic conditions means T = 298 K and P = 1 atm.).
The absolute entropy of Kr at 298.15 K is 163.97 J/mol-K. What is its absolute entropy at 200.00 K if the volume remains unchanged? Assume that the heat capacity is constant.
Calculate the change in molar entropy of graphite when heated from 0.0°C to 27°C. The constant pressure molar heat capacity fits the expression Cp,m /JK¹¹mol-¹ = 16.86 + 4.77 × 10³ K¹T-8.54 × 10-5 K²/T² between 240 K and 330 K.
2. Calculate the total molar entropy of HF at 298K. The vibrational frequency is 3960 cm-1 and the rotational constant is 20.6 cm-1.
Calculate the molar entropy of a constant-volume sample of argon at 270 K given that it is 154.84 J K–1 mol–1 at 298 K. Unit in J/mol-K.
The contributions to the molar heat capacity of a N2(g) at 273 K are: (A) Cv(translational) < Cv(rotational) < Cv(vibrational) (B) Cv(vibrational) < Cv(rotational) < Cv(translational) (C) Cv(rotational) < Cv(vibrational) < Cp(translational) (D) Cv(rotational) < Cv (translational) < Cv(vibrational)
) Given the following data on Phosphorus and its allotropeso ∆Hf kJ mol-1 ∆Gfo kJmol-1 So J mol-1 K-1 White phosphorus, P(s, white) 0 0 0 Gaseous Phosphorus, P(g) 315 278 163 Gaseous Phosphorus, P4(g) 59 24 280 b) For the transformation P(g) -> ¼ P4(g), is work done by the system or on the system? How much work is involved? Explainwith solutions. c) Calculate the ∆E in kJ for the process P(g)  ¼ P4(g) in (b). d) Calculate the sublimation temperature for white Phosphorus (in oC) assuming constant values of enthalpy and entropyover the temperature range involved.
7. The constant-volume molar heat capacity of a solid may be approximated by 3 12Tª Gy= 5 eD if T << ep. For Al, p = 398 K. What is the entropy change of a 5.0g mass of Al when it is heated at constant volume from 4 K to 176 K?
(c) [5 pts] Sketch a graph of the entropy of the van der Waals gas and the entropy of the perfect gas as a function of Vm for b = 1. What happens as b→ 0? Take n = 1 and plot S/nR. (d) [5 pts] Explain the intuition for the graph in (c) using the Boltzmann entropy and the number of microstates.